CH3OH(g)  CO(g) + 2 H2(g)   H = +90.7 kJ (a) Is the reaction exothermic or endothermic? exothermic endothermic     (b) Calculate the amount of heat transferred when 45.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. H = ____kJ (c) If the enthalpy change is 18.0 kJ, how many grams of hydrogen gas are produced? ____g

Consider the following reaction. (a) Is the reaction exothermic or endothermic? exothermic endothermic CH3OH(g) → CO(g) + 2 H₂(g) AH +90.7 kJ (b) Calculate the amount of heat transferred when 35.0 g of CH3OH(g) are decomposed by this reaction at constant pressure. ΔΗ= 100.8 (c) If the enthalpy change is 19.0 kJ, how many grams of hydrogen gas are produced? 0.42 x g (d) How many kilojoules of heat are released when 13.0 g of CO(g) reacts completely with H₂(g) to form CH₂OH(g) at constant pressure? AH = -90.7 X kJ (e) Calculate AE when 400.0 g of CH3OH(g) completely reacts at a constant temperature of 300 K and constant pressure of 0.95 atm. R = 8.314 J/mol*K and R = 0.08206 atm*L/mol K-41.7 XkJ HopHelpCh5N1

The common fertilizer NH,N0;(s), can explosively decompose according to the following reaction. What is the heat released when 80.06 g of NH,NO;(s) explodes? Molar mass of NH,NO:(s)= 80.06 g/mol. 28. 2 NH,NO3(s) → 2 N2(g) + O2(g)+4 H,O (g) AH = -236.15 kJ -472.3 kJ A) B) -236.15 kJ -118.08 kJ D) -59.04 kJ

In a popular television series, the two characters use thermite to assist with breaking into a chemical storage facility because the reaction between aluminum and iron(III) oxide produces a tremendous amount of heat. If they began with 10.0 g of Al, how many kJ of heat would be released? 29. 2 Al(s) + Fe,O3(s) → Al,O;(s) + 2 Fe(s) AH = -852 kJ 158 kJ A) B) 236 kJ 472 kJ D) None of the above

The sugar arabinose, C5 H10 O5, is burned completely in oxygen in a calorimeter. C5 H10 O5 (8) + 502(g) → 5CO2(g) + 5H2 O(1) Burning a 0.541 g sample caused the temperature to rise from 20.00°C to 20.54°C. The heat capacity of the calorimeter and its contents is 15.2 kJ/°C. Calculate AH for the combustion reaction per mole of arabinose. ΔΗ+ kJ/mol

What mass (in g) of fructose, when having undergone complete combustion, will release 6.13 x 102 kJ of heat? C,H12O6 (s) + 602(g) → 6CO2(g) + 6H2O(1) AH = -2.83 x 10° kJ mol-1 A: 39.0 aldnl nom

What is the mas of natural gas (CH4) must you burn to emit 276 kJ of heat?